Why does iodine have 3 lone pairs?

According to VSEPR theory, the central iodine atom has three equatorial lone pairs, and the terminal iodine atoms are bonded axially in a linear fashion, due to the three lone pairs bonding to the central iodine-atom.

What is the total number of lone pairs in the best Lewis structure for ICl2 I is the central atom )?

3 lone pairs
Therefore, In the Lewis structure of $ICl_2^ -$, 3 lone pairs of electrons are around the iodine atom.

Does iodine have any lone pairs?

An iodine atom has 3 lone pairs of electrons.

Is ICl2 polar or nonpolar?

$ IC{l_2}^ – $ is a nonpolar molecule. $ IC{l_2}^ – $ with 22 valence electrons has 3 lone pairs and 2 shared pairs of the central $ I $ atom and the linear shape is non-polar because the dipoles cancel out each other giving net dipole moment zero.

Why is ICl2 linear?

While there are 3 atoms in $IC{l_2}^ – $in a line in the z-plane. As we know that the structure of $IC{l_2}^ – $is linear with a lone pair. So, it makes it trigonal bipyramidal but as there are two three lone pair electrons so it makes it linear in structure with a hybridization of $s{p^3}d$.

How many lone pairs does the Lewis dot structure of iodine have?

Iodine is a diatomic molecule and contains only two iodine atoms. Lewis structure of iodine molecule contains only one I-I bond and each iodine atom has three lone pairs.

What is the formal charge on the iodine in ICl2?

So this is the Lewis structure for ICl2-. If you check the formal charges, you’ll note that there is a negative charge on the Iodine and the Chlorines both have a formal charge of zero.

Why is ICl2 nonpolar and ICl2 is polar?

Because of the opposing charges, a polar molecule has a net dipole. $ IC{l_2}^ – $ is a nonpolar molecule. $ IC{l_2}^ – $ with 22 valence electrons has 3 lone pairs and 2 shared pairs of the central $ I $ atom and the linear shape is non-polar because the dipoles cancel out each other giving net dipole moment zero.